Standard electrode potential (data page)

Main article: Standard electrode potential

The data below tabulates standard electrode potentials (E°), in volts relative to the standard hydrogen electrode (SHE), at:

• Temperature 298.15 K (25.00 °C; 77.00 °F);
• Effective concentration (activity) 1 mol/L for each aqueous or amalgamated (mercury-alloyed) species;
• Unit activity for each solvent and pure solid or liquid species; and
• Absolute partial pressure 101.325 kPa (1.00000 atm; 1.01325 bar) for each gaseous reagent — the convention in most literature data but not the current standard state (100 kPa).

Variations from these ideal conditions affect measured voltage via the Nernst equation.

Electrode potentials of successive elementary half-reactions cannot be directly added. However, the corresponding Gibbs free energy changes (∆G°) must satisfy

∆G° = –zFE°,

where z electrons are transferred, and the Faraday constant F is the conversion factor describing Coulombs transferred per mole electrons. Those Gibbs free energy changes can be added.

For example, from Fe^2+ + 2 e^− ⇌ Fe(s) (–0.44 V), the energy to form one neutral atom of Fe(s) from one Fe^2+ ion and two electrons is 2 × 0.44 eV = 0.88 eV, or 84 907 J/(mol  e^−). That value is also the standard formation energy (∆G_f°) for an Fe^2+ ion, since  e^− and Fe(s) both have zero formation energy.

Data from different sources may cause table inconsistencies. For example: $${\displaystyle {\begin{alignedat}{4}&{\ce {Cu+ + e-}}&{}\rightleftharpoons {}&{\ce {Cu(s)}}&\quad \quad E_{1}=+0.520{\text{ V}}\\&{\ce {Cu^2+ + 2e-}}&{}\rightleftharpoons {}&{\ce {Cu(s)}}&\quad \quad E_{2}=+0.337{\text{ V}}\\&{\ce {Cu^2+ + e-}}&{}\rightleftharpoons {}&{\ce {Cu+}}&\quad \quad E_{3}=+0.159{\text{ V}}\end{alignedat}}}$$ From additivity of Gibbs energies, one must have $${\displaystyle 2\cdot E_{2}=1\cdot E_{1}+1\cdot E_{3}}$$ But that equation does not hold exactly with the cited values.

Table of standard electrode potentials

Legend: (s) – solid; (l) – liquid; (g) – gas; (aq) – aqueous (default for all charged species); (Hg) – amalgam; bold – water electrolysis equations.

Element	Half-reaction			E° (volt)	Electrons transferred	Reference
	Oxidant	⇌	Reductant
Sr	Sr^+ +  e^−	⇌	Sr(s)	-4.101	1
Ca	Ca^+ +  e^−	⇌	Ca(s)	-3.8	1
Th	Th^4+ +  e^−	⇌	Th^3+	-3.6	1
Pr	Pr^3+ +  e^−	⇌	Pr^2+	-3.1	1
N	3N 2(g) + 2 H^+ + 2 e^−	⇌	2HN 3(aq)	-3.09	2
Li	Li^+ +  e^−	⇌	Li(s)	-3.0401	1
N	N 2(g) + 4H2O + 2 e^−	⇌	2NH 2OH(aq) + 2 OH^−	-3.04	2
Cs	Cs^+ +  e^−	⇌	Cs(s)	-3.026	1
Ca	Ca(OH) 2 + 2 e^−	⇌	Ca(s) + 2 OH^−	-3.02	2
Er	Er^3+ +  e^−	⇌	Er^2+	-3	1
Ba	Ba(OH) 2 + 2 e^−	⇌	Ba(s) + 2 OH^−	-2.99	2
Rb	Rb^+ +  e^−	⇌	Rb(s)	-2.98	1
K	K^+ +  e^−	⇌	K(s)	-2.931	1
Ba	Ba^2+ + 2 e^−	⇌	Ba(s)	-2.912	2
La	La(OH) 3(s) + 3 e^−	⇌	La(s) + 3 OH^−	-2.9	3
Fr	Fr^+ +  e^−	⇌	Fr(s)	-2.9	1
Sr	Sr^2+ + 2 e^−	⇌	Sr(s)	-2.899	2
Sr	Sr(OH) 2 + 2 e^−	⇌	Sr(s) + 2 OH^−	-2.88	2
Ca	Ca^2+ + 2 e^−	⇌	Ca(s)	-2.868	2
Li	Li^+ + C 6(s) +  e^−	⇌	LiC 6(s)	-2.84	1
Eu	Eu^2+ + 2 e^−	⇌	Eu(s)	-2.812	2
Ra	Ra^2+ + 2 e^−	⇌	Ra(s)	-2.8	2
Ho	Ho^3+ +  e^−	⇌	Ho^2+	-2.8	1
Bk	Bk^3+ +  e^−	⇌	Bk^2+	-2.8	1
Yb	Yb^2+ + 2 e^−	⇌	Yb(s)	-2.76	2
Na	Na^+ +  e^−	⇌	Na(s)	-2.71	1
Mg	Mg^+ +  e^−	⇌	Mg(s)	-2.7	1
Nd	Nd^3+ +  e^−	⇌	Nd^2+	-2.7	1
Mg	Mg(OH) 2 + 2 e^−	⇌	Mg(s) + 2 OH^−	-2.69	2
Sm	Sm^2+ + 2 e^−	⇌	Sm(s)	-2.68	2
Be	Be 2O^2− 3 + 3H2O + 4 e^−	⇌	2Be(s) + 6 OH^−	-2.63	4
Pm	Pm^3+ +  e^−	⇌	Pm^2+	-2.6	1
Dy	Dy^3+ +  e^−	⇌	Dy^2+	-2.6	1
No	No^2+ + 2 e^−	⇌	No	-2.5	2
Hf	HfO(OH) 2 + H2O + 4 e^−	⇌	Hf(s) + 4 OH^−	-2.5	4
Th	Th(OH) 4 + 4 e^−	⇌	Th(s) + 4 OH^−	-2.48	4
Md	Md^2+ + 2 e^−	⇌	Md	-2.4	2
Tm	Tm^2+ + 2 e^−	⇌	Tm(s)	-2.4	2
La	La^3+ + 3 e^−	⇌	La(s)	-2.379	3
Y	Y^3+ + 3 e^−	⇌	Y(s)	-2.372	3
Mg	Mg^2+ + 2 e^−	⇌	Mg(s)	-2.372	2
Sc	ScF3(aq) + 3 H^+ + 3 e^−	⇌	Sc(s) + 3HF(aq)	-2.37	3
Zr	ZrO(OH) 2(s) + H2O + 4 e^−	⇌	Zr(s) + 4 OH^−	-2.36	4
Pr	Pr^3+ + 3 e^−	⇌	Pr(s)	-2.353	3
Ce	Ce^3+ + 3 e^−	⇌	Ce(s)	-2.336	3
Er	Er^3+ + 3 e^−	⇌	Er(s)	-2.331	3
Ho	Ho^3+ + 3 e^−	⇌	Ho(s)	-2.33	3
Al	H 2AlO^− 3 + H2O + 3 e^−	⇌	Al(s) + 4 OH^−	-2.33	3
Nd	Nd^3+ + 3 e^−	⇌	Nd(s)	-2.323	3
Tm	Tm^3+ + 3 e^−	⇌	Tm(s)	-2.319	3
Al	Al(OH) 3(s) + 3 e^−	⇌	Al(s) + 3 OH^−	-2.31	3
Sm	Sm^3+ + 3 e^−	⇌	Sm(s)	-2.304	3
Fm	Fm^2+ + 2 e^−	⇌	Fm	-2.3	2
Am	Am^3+ +  e^−	⇌	Am^2+	-2.3	1
Dy	Dy^3+ + 3 e^−	⇌	Dy(s)	-2.295	3
Lu	Lu^3+ + 3 e^−	⇌	Lu(s)	-2.28	3
Sc	ScF^+ 2 + 2 H^+ + 3 e^−	⇌	Sc(s) + 2HF(l)	-2.28	3
Tb	Tb^3+ + 3 e^−	⇌	Tb(s)	-2.28	3
Gd	Gd^3+ + 3 e^−	⇌	Gd(s)	-2.279	3
H	H 2(g) + 2 e^−	⇌	2H^−	-2.23	2
Es	Es^2+ + 2 e^−	⇌	Es(s)	-2.23	2
Pm	Pm^2+ + 2 e^−	⇌	Pm(s)	-2.2	2
Tm	Tm^3+ +  e^−	⇌	Tm^2+	-2.2	1
Dy	Dy^2+ + 2 e^−	⇌	Dy(s)	-2.2	2
Ac	Ac^3+ + 3 e^−	⇌	Ac(s)	-2.2	3
Yb	Yb^3+ + 3 e^−	⇌	Yb(s)	-2.19	3
Cf	Cf^2+ + 2 e^−	⇌	Cf(s)	-2.12	2
Nd	Nd^2+ + 2 e^−	⇌	Nd(s)	-2.1	2
Ho	Ho^2+ + 2 e^−	⇌	Ho(s)	-2.1	2
Sc	Sc^3+ + 3 e^−	⇌	Sc(s)	-2.077	3
Al	AlF^3− 6 + 3 e^−	⇌	Al(s) + 6F^−	-2.069	3
Cm	Cm^3+ + 3 e^−	⇌	Cm(s)	-2.04	3
Pu	Pu^3+ + 3 e^−	⇌	Pu(s)	-2.031	3
Pr	Pr^2+ + 2 e^−	⇌	Pr(s)	-2	2
Er	Er^2+ + 2 e^−	⇌	Er(s)	-2	2
Eu	Eu^3+ + 3 e^−	⇌	Eu(s)	-1.991	3
Lr	Lr^3+ + 3 e^−	⇌	Lr	-1.96	3
Cf	Cf^3+ + 3 e^−	⇌	Cf(s)	-1.94	3
Es	Es^3+ + 3 e^−	⇌	Es(s)	-1.91	3
Pa	Pa^4+ +  e^−	⇌	Pa^3+	-1.9	1
Am	Am^2+ + 2 e^−	⇌	Am(s)	-1.9	2
Th	Th^4+ + 4 e^−	⇌	Th(s)	-1.899	4
Fm	Fm^3+ + 3 e^−	⇌	Fm	-1.89	3
N	N2(g) + 2H2O(l) + 4 H^+ + 2 e^−	⇌	2NH3OH^+	-1.87	2
Np	Np^3+ + 3 e^−	⇌	Np(s)	-1.856	3
Be	Be^2+ + 2 e^−	⇌	Be(s)	-1.847	2
P	H 2PO^− 2 +  e^−	⇌	P(s) + 2 OH^−	-1.82	1
U	U^3+ + 3 e^−	⇌	U(s)	-1.798	3
Sr	Sr^2+ + 2 e^−	⇌	Sr(Hg)	-1.793	2
B	H 2BO^− 3 + H2O + 3 e^−	⇌	B(s) + 4 OH^−	-1.79	3
Th	ThO 2 + 4 H^+ + 4 e^−	⇌	Th(s) + 2H2O	-1.789	4
Hf	HfO^2+ + 2 H^+ + 4 e^−	⇌	Hf(s) + H2O	-1.724	4
P	HPO^2− 3 + 2H2O + 3 e^−	⇌	P(s) + 5 OH^−	-1.71	3
Si	SiO^2− 3 + 3H2O + 4 e^−	⇌	Si(s) + 6 OH^−	-1.697	4
Al	Al^3+ + 3 e^−	⇌	Al(s)	-1.662	3
Ti	Ti^2+ + 2 e^−	⇌	Ti(s)	-1.63	2
Zr	ZrO 2(s) + 4 H^+ + 4 e^−	⇌	Zr(s) + 2H2O	-1.553	4
Zr	Zr^4+ + 4 e^−	⇌	Zr(s)	-1.45	4
Ti	Ti^3+ + 3 e^−	⇌	Ti(s)	-1.37	3
Ti	TiO(s) + 2 H^+ + 2 e^−	⇌	Ti(s) + H2O	-1.31	2
B	B(OH)^− 4 + 4H2O(l) + 8 e^−	⇌	BH^− 4 + 8 OH^−	-1.24	8
Ga	GaO(OH)^− 2 + H2O(l) + 3 e^−	⇌	Ga(s) + 3 OH^−	-1.22	3
Ti	Ti 2O 3(s) + 2 H^+ + 2 e^−	⇌	2TiO(s) + H2O	-1.23	2
Zn	Zn(OH)^2− 4 + 2 e^−	⇌	Zn(s) + 4 OH^−	-1.199	2
Mn	Mn^2+ + 2 e^−	⇌	Mn(s)	-1.185	2
Fe	Fe(CN)^4− 6 + 6 H^+ + 2 e^−	⇌	Fe(s) + 6HCN(aq)	-1.16	2
C	C(s) + 3H2O(l) + 2 e^−	⇌	CH3OH(l) + 2 OH^−	-1.148	2
Cr	Cr(CN)^3− 6 +  e^−	⇌	Cr(CN)^4− 6	-1.143	1
Te	Te(s) + 2 e^−	⇌	Te^2−	-1.143	2
V	V^2+ + 2 e^−	⇌	V(s)	-1.13	2
Nb	Nb^3+ + 3 e^−	⇌	Nb(s)	-1.099	3
Sn	Sn(s) + 4 H^+ + 4 e^−	⇌	SnH 4(g)	-1.07	4
Po	Po(s) + 2 e^−	⇌	Po^2−	-1.021	2
Cr	[Cr(edta)(H2O)]^− +  e^−	⇌	[Cr(edta)(H2O)]^2−	-0.99	1
P	2H3PO4(aq) + 2 H^+ + 2 e^−	⇌	(H2PO3)2(aq) + H2O(l)	-0.933	2
C	CO^2− 3 + 3 H^+ + 2 e^−	⇌	HCO^− 2 + H2O(l)	-0.93	2
Ti	TiO^2+ + 2 H^+ + 4 e^−	⇌	Ti(s) + H2O	-0.93	4
Si	SiO 2(quartz) + 4 H^+ + 4 e^−	⇌	Si(s) + 2H2O	-0.909	4
Cr	Cr^2+ + 2 e^−	⇌	Cr(s)	-0.9	2
B	B(OH) 3(aq) + 3 H^+ + 3 e^−	⇌	B(s) + 3H2O	-0.89	3
Fe	Fe(OH) 2(s) + 2 e^−	⇌	Fe(s) + 2 OH^−	-0.89	2
Fe	Fe 2O 3(s) + 3H2O + 2 e^−	⇌	2Fe(OH) 2(s) + 2 OH^−	-0.86	2
H	2H2O + 2 e^−	⇌	H 2(g) + 2 OH^−	-0.8277	2
Bi	Bi(s) + 3 H^+ + 3 e^−	⇌	BiH 3	-0.8	3
Zn	Zn^2+ + 2 e^−	⇌	Zn(Hg)	-0.7628	2
Zn	Zn^2+ + 2 e^−	⇌	Zn(s)	-0.7618	2
Ta	Ta 2O 5(s) + 10 H^+ + 10 e^−	⇌	2Ta(s) + 5H2O	-0.75	10
Te	2Te(s) + 2 e^−	⇌	Te^2− 2	-0.74	2
Ni	Ni(OH) 2(s) + 2 e^−	⇌	Ni(s) + 2 OH^−	-0.72	2
Nb	Nb2O5(s) + 10 H^+ + 10 e^−	⇌	2Nb(s) + 5H2O(l)	-0.7	10
Ag	Ag 2S(s) + 2 e^−	⇌	2Ag(s) + S^2− (aq)	-0.69	2
Te	Te^2− 2 + 4 H^+ + 2 e^−	⇌	2H2Te(g)	-0.64	2
Sb	Sb(OH)^− 4 + 3 e^−	⇌	Sb(s) + 4 OH^−	-0.639	3
Au	[Au(CN) 2]^− +  e^−	⇌	Au(s) + 2CN^−	-0.6	1
Ta	Ta^3+ + 3 e^−	⇌	Ta(s)	-0.6	3
Pb	PbO(s) + H2O + 2 e^−	⇌	Pb(s) + 2 OH^−	-0.580	2
Ti	2TiO 2(s) + 2 H^+ + 2 e^−	⇌	Ti 2O 3(s) + H2O	-0.56	2
Ga	Ga^3+ + 3 e^−	⇌	Ga(s)	-0.549	3
U	U^4+ +  e^−	⇌	U^3+	-0.52	1
P	H 3PO 2(aq) +  H^+ +  e^−	⇌	P(white)[note 1] + 2H2O	-0.508	1
P	H 3PO 3(aq) + 2 H^+ + 2 e^−	⇌	H 3PO 2(aq) + H2O	-0.499	2
Ni	NiO 2(s) + 2H2O + 2 e^−	⇌	Ni(OH) 2(s) + 2 OH^−	-0.49	2
Sb	Sb(OH)^− 6 + 2 e^−	⇌	Sb(OH)^− 4 + 2 OH^−	-0.465	2
P	H 3PO 3(aq) + 3 H^+ + 3 e^−	⇌	P(red)[note 1] + 3H2O	-0.454	3
Bi	Bi2O3(s) + 3H2O(l) + 6 e^−	⇌	Bi(s) + 6 OH^−	-0.452	6
Ta	TaF^2− 7 + 7 H^+ + 5 e^−	⇌	Ta(s) + 7HF(l)	-0.45	5
In	In^3+ + 2 e^−	⇌	In^+	-0.444	2
Cu	Cu(CN)^− 2 +  e^−	⇌	Cu(s) + 2CN^−	-0.44	1
Fe	Fe^2+ + 2 e^−	⇌	Fe(s)	-0.44	2
C	2CO 2(g) + 2 H^+ + 2 e^−	⇌	HOOCCOOH(aq)	-0.43	2
Cr	Cr^3+ +  e^−	⇌	Cr^2+	-0.407	1
Cd	Cd^2+ + 2 e^−	⇌	Cd(s)	-0.4	2
Ti	Ti^3+ +  e^−	⇌	Ti^2+	-0.37	1
Cu	Cu 2O(s) + H2O + 2 e^−	⇌	2Cu(s) + 2 OH^−	-0.36	2
Pb	PbSO 4(s) + 2 e^−	⇌	Pb(s) + SO^2− 4	-0.3588	2
Pb	PbSO 4(s) + 2 e^−	⇌	Pb(Hg) + SO^2− 4	-0.3505	2
Eu	Eu^3+ +  e^−	⇌	Eu^2+	-0.35	1
In	In^3+ + 3 e^−	⇌	In(s)	-0.34	3
Tl	Tl^+ +  e^−	⇌	Tl(s)	-0.34	1
Ge	Ge(s) + 4 H^+ + 4 e^−	⇌	GeH 4(g)	-0.29	4
Co	Co^2+ + 2 e^−	⇌	Co(s)	-0.28	2
P	H 3PO 4(aq) + 2 H^+ + 2 e^−	⇌	H 3PO 3(aq) + H2O	-0.276	2
N	N2(g) + 8 H^+ + 6 e^−	⇌	2NH^+ 4	-0.27	6
V	V^3+ +  e^−	⇌	V^2+	-0.26	1
Ni	Ni^2+ + 2 e^−	⇌	Ni(s)	-0.257	2
S	2HSO^− 4 + 2 H^+ + 2 e^−	⇌	S2O^2− 6 + 2H2O(l)	-0.253	2
As	As(s) + 3 H^+ + 3 e^−	⇌	AsH 3(g)	-0.23	3
N	N2(g) + 5 H^+ + 4 e^−	⇌	N2H^+ 5	-0.23	4
Ga	Ga^+ +  e^−	⇌	Ga(s)	-0.2	1
Ag	AgI(s) +  e^−	⇌	Ag(s) + I^−	-0.15224	1
Ge	GeO2(s) + 4 H^+ + 4 e^−	⇌	Ge(s) + 2H2O(l)	-0.15	4
Mo	MoO 2(s) + 4 H^+ + 4 e^−	⇌	Mo(s) + 2H2O	-0.15	4
Si	Si(s) + 4 H^+ + 4 e^−	⇌	SiH 4(g)	-0.14	4
Sn	Sn^2+ + 2 e^−	⇌	Sn(s)	-0.13	2
O	O 2(g) +  H^+ +  e^−	⇌	HO^• 2(aq)	-0.13	1
In	In^+ +  e^−	⇌	In(s)	-0.126	1
Pb	Pb^2+ + 2 e^−	⇌	Pb(s)	-0.126	2
W	WO 2(s) + 4 H^+ + 4 e^−	⇌	W(s) + 2H2O	-0.12	4
Ge	GeO 2(s) + 2 H^+ + 2 e^−	⇌	GeO(s) + H2O	-0.118	2
P	P(red) + 3 H^+ + 3 e^−	⇌	PH 3(g)	-0.111	3
C	CO 2(g) + 2 H^+ + 2 e^−	⇌	HCOOH(aq)	-0.11	2
Se	Se(s) + 2 H^+ + 2 e^−	⇌	H 2Se(g)	-0.11	2
C	CO 2(g) + 2 H^+ + 2 e^−	⇌	CO(g) + H2O	-0.11	2
Sn	α-SnO(s) + 2 H^+ + 2 e^−	⇌	Sn(s) + H2O	-0.104	2
Cu	Cu(NH 3)^+ 2 +  e^−	⇌	Cu(s) + 2NH 3(aq)	-0.1	1
Nb	Nb2O5(s) + 10 H^+ + 4 e^−	⇌	2Nb^3+ + 5H2O(l)	-0.1	4
W	WO 3(aq) + 6 H^+ + 6 e^−	⇌	W(s) + 3H2O	-0.09	6
Sn	SnO 2(s) + 2 H^+ + 2 e^−	⇌	α-SnO(s) + H2O	-0.088	2
Fe	Fe 3O 4(s) + 8 H^+ + 8 e^−	⇌	3Fe(s) + 4H2O	-0.085	8
V	VOH^2+ +  H^+ +  e^−	⇌	V^2+ + H2O(l)	-0.082	1
P	P(white) + 3 H^+ + 3 e^−	⇌	PH 3(g)	-0.063	3
N	N2O(g) + H2O(l) + 6 H^+ + 4 e^−	⇌	2NH3OH^+	-0.05	4
Fe	Fe^3+ + 3 e^−	⇌	Fe(s)	-0.04	3
C	HCOOH(aq) + 2 H^+ + 2 e^−	⇌	HCHO(aq) + H2O	-0.034	2
H	2 H^+ + 2 e^−	⇌	H 2(g)	0	2
Ag	AgBr(s) +  e^−	⇌	Ag(s) + Br^−	0.07133	1
S	S 4O^2− 6 + 2 e^−	⇌	2S 2O^2− 3	0.08	2
N	N 2(g) + 2H2O + 6 H^+ + 6 e^−	⇌	2NH 4OH(aq)	0.092	6
Hg	HgO(s) + H2O + 2 e^−	⇌	Hg(l) + 2 OH^−	0.0977	2
Cu	Cu(NH 3)^2+ 4 +  e^−	⇌	Cu(NH 3)^+ 2 + 2NH 3(aq)	0.1	1
Ru	Ru(NH 3)^3+ 6 +  e^−	⇌	Ru(NH 3)^2+ 6	0.1	1
N	N 2H 4(aq) + 4H2O + 2 e^−	⇌	2NH^+ 4 + 4 OH^−	0.11	2
Mo	H 2MoO 4(aq) + 6 H^+ + 6 e^−	⇌	Mo(s) + 4H2O	0.11	6
Ge	Ge^4+ + 4 e^−	⇌	Ge(s)	0.12	4
C	C(s) + 4 H^+ + 4 e^−	⇌	CH 4(g)	0.13	4
C	HCHO(aq) + 2 H^+ + 2 e^−	⇌	CH 3OH(aq)	0.13	2
S	S(s) + 2 H^+ + 2 e^−	⇌	H 2S(g)	0.144	2
Sb	Sb2O3(s) + 6 H^+ + 6 e^−	⇌	2Sb(s) + 3H2O	0.15	6	[6]: 789
Sn	Sn^4+ + 2 e^−	⇌	Sn^2+	0.151	2
S	HSO^− 4 + 3 H^+ + 2 e^−	⇌	SO 2(aq) + 2H2O	0.158	2
Cu	Cu^2+ +  e^−	⇌	Cu^+	0.159	1
U	UO^2+ 2 +  e^−	⇌	UO^+ 2	0.163	1
S	SO^2− 4 + 4 H^+ + 2 e^−	⇌	SO 2(aq) + 2H2O	0.17	2
Ti	TiO^2+ + 2 H^+ +  e^−	⇌	Ti^3+ + H2O	0.19	1
Sb	SbO^+ + 2 H^+ + 3 e^−	⇌	Sb(s) + H2O	0.2	3
Fe	3Fe 2O 3(s) + 2 H^+ + 2 e^−	⇌	2Fe 3O 4(s) + H2O	0.22	2
Ag	AgCl(s) +  e^−	⇌	Ag(s) + Cl^−	0.22233	1
As	H 3AsO 3(aq) + 3 H^+ + 3 e^−	⇌	As(s) + 3H2O	0.24	3
Ru	Ru^3+ (aq) +  e^−	⇌	Ru^2+ (aq)	0.249	1
Pb	PbO2(s) + H2O + 2 e^−	⇌	α-PbO(s) + 2 OH^−	0.254	2
Ge	GeO(s) + 2 H^+ + 2 e^−	⇌	Ge(s) + H2O	0.26	2
Hg	Hg2Cl2(s) + 2 e^−	⇌	2Hg(l) + 2Cl^−	0.27	2
U	UO^+ 2 + 4 H^+ +  e^−	⇌	U^4+ + 2H2O	0.273	1
Re	Re^3+ + 3 e^−	⇌	Re(s)	0.300	3
At	At +  e^−	⇌	At^−	0.3	1
Bi	Bi^3+ + 3 e^−	⇌	Bi(s)	0.308	3
C	2HCNO + 2 H^+ + 2 e^−	⇌	(CN)2 + 2H2O	0.330	2
Cu	Cu^2+ + 2 e^−	⇌	Cu(s)	0.337	2
V	VO^2+ + 2 H^+ +  e^−	⇌	V^3+ + H2O	0.337	1
Sb	Sb2O4(s) + 2 H^+ + 2 e^−	⇌	Sb2O3(s) + H2O(l)	0.342	2
At	At^+ + 2 e^−	⇌	At^−	0.36	2
Fe	[Fe(CN) 6]^3− +  e^−	⇌	[Fe(CN) 6]^4−	0.3704	1
C	(CN)2 + 2 H^+ + 2 e^−	⇌	2HCN	0.373	2
P	(H2PO3)2(aq) + 2 H^+ + 2 e^−	⇌	2H3PO3	0.38	2
S	2SO2(aq) + 2 H^+ + 2 e^−	⇌	S2O^2− 3 + H2O(l)	0.4	2
O	O 2(g) + 2H2O + 4 e^−	⇌	4 OH^−(aq)	0.401	4
Mo	H 2MoO 4 + 6 H^+ + 3 e^−	⇌	Mo^3+ + 4H2O	0.43	3
Ru	Ru^2+ (aq) + 2 e^−	⇌	Ru	0.455	2
V	VO(OH)^+ + 2 H^+ +  e^−	⇌	VOH^2+ + H2O(l)	0.481	1
C	CH 3OH(aq) + 2 H^+ + 2 e^−	⇌	CH 4(g) + H2O	0.5	2
S	SO 2(aq) + 4 H^+ + 4 e^−	⇌	S(s) + 2H2O	0.5	4
S	4SO 2(aq) + 4 H^+ + 8 e^−	⇌	S4O^2− 6 + 2H2O(l)	0.51	8
Cu	Cu^+ +  e^−	⇌	Cu(s)	0.52	1
C	CO(g) + 2 H^+ + 2 e^−	⇌	C(s) + H2O	0.52	2
I	I^− 3 + 2 e^−	⇌	3I^−	0.53	2
Te	TeO2(s) + 4 H^+ + 4 e^−	⇌	Te(s) + 2H2O(l)	0.53	4
Cu	Cu^2+ + Cl^− +  e^−	⇌	CuCl(s)	0.54	1
I	I 2(s) + 2 e^−	⇌	2I^−	0.54	2
Au	[AuI 4]^− + 3 e^−	⇌	Au(s) + 4I^−	0.56	3
As	H 3AsO 4(aq) + 2 H^+ + 2 e^−	⇌	H 3AsO 3(aq) + H2O	0.56	2
S	S2O^2− 6 + 4 H^+ + 2 e^−	⇌	2H2SO3	0.569	2
Au	[AuI 2]^− +  e^−	⇌	Au(s) + 2I^−	0.58	1
Mn	MnO^− 4 + 2H2O + 3 e^−	⇌	MnO 2(s) + 4 OH^−	0.595	3
S	S 2O^2− 3 + 6 H^+ + 4 e^−	⇌	2S(s) + 3H2O	0.6	4
Fe	Fc^+ +  e^−	⇌	Fc(s)	0.63	1
Mo	H 2MoO 4(aq) + 2 H^+ + 2 e^−	⇌	MoO 2(s) + 2H2O	0.65	2
N	HN3(aq) + 11 H^+ + 8 e^−	⇌	3NH^+ 4	0.69	8
O	O 2(g) + 2 H^+ + 2 e^−	⇌	H 2O 2(aq)	0.695	2
Sb	Sb2O5(s) + 4 H^+ + 4 e^−	⇌	Sb2O3(s) + 2H2O	0.699	4
C	+ 2 H^+ + 2 e^−	⇌		0.6992	2
V	H2V10O^4− 28 + 24 H^+ + 10 e^−	⇌	10VO(OH)^+ + 8H2O(l)	0.723	10
Pt	PtCl^2− 6 + 2 e^−	⇌	PtCl^2− 4 + 2Cl^−	0.726	2
Fe	Fe 2O 3(s) + 6 H^+ + 2 e^−	⇌	2Fe^2+ + 3H2O	0.728	2
Se	H 2SeO 3(aq) + 4 H^+ + 4 e^−	⇌	Se(s) + 3H2O	0.74	4
At	AtO^+ + 2 H^+ + 2 e^−	⇌	At^+ + H2O	0.74	2
Tl	Tl^3+ + 3 e^−	⇌	Tl(s)	0.741	3
No	No^3+ +  e^−	⇌	No^2+	0.75	1
Pt	PtCl^2− 4 + 2 e^−	⇌	Pt(s) + 4Cl^−	0.758	2
Br	BrO^− + H2O(l) + 2 e^−	⇌	Br^− + 2 OH^−	0.76	2
Po	Po^4+ + 4 e^−	⇌	Po	0.76	4
S	(SCN)2 + 2 e^−	⇌	2SCN^−	0.769	2
Fe	Fe^3+ +  e^−	⇌	Fe^2+	0.771	1
Hg	Hg^2+ 2 + 2 e^−	⇌	2Hg(l)	0.7973	2
Ag	Ag^+ +  e^−	⇌	Ag(s)	0.7996	1
N	2NO^− 3(aq) + 4 H^+ + 2 e^−	⇌	N 2O 4(g) + 2H2O	0.803	2
Fe	2FeO^2− 4 + 5H2O + 6 e^−	⇌	Fe 2O 3(s) + 10 OH^−	0.81	6
Au	[AuBr 4]^− + 3 e^−	⇌	Au(s) + 4Br^−	0.85	3
Hg	Hg^2+ + 2 e^−	⇌	Hg(l)	0.85	2
Ir	[IrCl 6]^2− +  e^−	⇌	[IrCl 6]^3−	0.87	1
Mn	MnO^− 4 +  H^+ +  e^−	⇌	HMnO^− 4	0.9	1
Po	Po^4+ + 2 e^−	⇌	Po^2+	0.9	2
Hg	2Hg^2+ + 2 e^−	⇌	Hg^2+ 2	0.91	2
Pd	Pd^2+ + 2 e^−	⇌	Pd(s)	0.915	2
Au	[AuCl 4]^− + 3 e^−	⇌	Au(s) + 4Cl^−	0.93	3
N	NO^− 3 + 3 H^+ + 2 e^−	⇌	HNO2(aq)	0.94	2
Mn	MnO 2(s) + 4 H^+ +  e^−	⇌	Mn^3+ + 2H2O	0.95	1
N	NO^− 3(aq) + 4 H^+ + 3 e^−	⇌	NO(g) + 2H2O(l)	0.958	3
Au	[AuBr 2]^− +  e^−	⇌	Au(s) + 2Br^−	0.96	1
Fe	Fe 3O 4(s) + 8 H^+ + 2 e^−	⇌	3Fe^2+ + 4H2O	0.98	2
Xe	[HXeO 6]^3− + 2H2O + 2 e^−	⇌	[HXeO 4]^− + 4 OH^−	0.99	2
N	HNO2(aq) +  H^+ +  e^−	⇌	NO(g) + H2O(l)	0.996	1
At	HAtO +  H^+ +  e^−	⇌	At + H2O	1.0	1
V	[VO 2]^+ (aq) + 2 H^+ +  e^−	⇌	[VO]^2+ (aq) + H2O	1	1
Te	H 6TeO 6(aq) + 2 H^+ + 2 e^−	⇌	TeO 2(s) + 4H2O	1.02	2
N	NO2(g) + 2 H^+ + 2 e^−	⇌	NO(g) + H2O(l)	1.03	2
Br	Br^− 3 + 2 e^−	⇌	3Br^−	1.05	2
Sb	Sb2O5(s) + 2 H^+ + 2 e^−	⇌	Sb2O4(s) + H2O(l)	1.055	2
I	ICl^− 2 +  e^−	⇌	2Cl^− + I(s)	1.06	1
Br	Br 2(l) + 2 e^−	⇌	2Br^−	1.066	2
N	N2O4(g) + 2 H^+ + 2 e^−	⇌	2HNO2	1.07	2
Br	Br 2(aq) + 2 e^−	⇌	2Br^−	1.0873	2
Ru	RuO 2 + 4 H^+ + 2 e^−	⇌	Ru^2+ (aq) + 2H2O	1.120	2
Cu	Cu^2+ + 2CN^− +  e^−	⇌	Cu(CN)^− 2	1.12	1
I	IO^− 3 + 5 H^+ + 4 e^−	⇌	HIO(aq) + 2H2O	1.13	4
O	H2O2(aq) +  H^+ +  e^−	⇌	H2O(l) + HO•	1.14	1
Au	[AuCl 2]^− +  e^−	⇌	Au(s) + 2Cl^−	1.15	1
Se	HSeO^− 4 + 3 H^+ + 2 e^−	⇌	H 2SeO 3(aq) + H2O	1.15	2
Ag	Ag 2O(s) + 2 H^+ + 2 e^−	⇌	2Ag(s) + H2O	1.17	2
Cl	ClO^− 3 + 2 H^+ +  e^−	⇌	ClO 2(g) + H2O	1.175	1
Xe	[HXeO 6]^3− + 5H2O + 8 e^−	⇌	Xe(g) + 11 OH^−	1.18	8
Pt	Pt^2+ + 2 e^−	⇌	Pt(s)	1.188	2
Cl	ClO 2(g) +  H^+ +  e^−	⇌	HClO 2(aq)	1.19	1
I	2IO^− 3 + 12 H^+ + 10 e^−	⇌	I 2(s) + 6H2O	1.2	10
Mn	MnO 2(s) + 4 H^+ + 2 e^−	⇌	Mn^2+ + 2H2O	1.224	2
O	O 2(g) + 4 H^+ + 4 e^−	⇌	2H2O	1.229	4
N	N2H^+ 5 + 3 H^+ + 2 e^−	⇌	2NH^+ 4	1.28	2
Cl	ClO^− 4 + 2 H^+ + 2 e^−	⇌	ClO^− 3 + H2O	1.23	2
Ru	[Ru(bipy) 3]^3+ +  e^−	⇌	[Ru(bipy) 3]^2+	1.24	1
Xe	[HXeO 4]^− + 3H2O + 6 e^−	⇌	Xe(g) + 7 OH^−	1.24	6
N	2NO^− 3 + 12 H^+ + 10 e^−	⇌	N2(g) + 6H2O(l)	1.25	10
Tl	Tl^3+ + 2 e^−	⇌	Tl^+	1.25	2
N	2HNO2(aq) + 4 H^+ + 4 e^−	⇌	N2O(g) + 3H2O(l)	1.297	4
Cr	Cr 2O^2− 7 + 14 H^+ + 6 e^−	⇌	2Cr^3+ + 7H2O	1.33	6
N	NH3OH^+ + 2 H^+ + 2 e^−	⇌	NH^+ 4 + H2O(l)	1.35	2
Cl	Cl 2(g) + 2 e^−	⇌	2Cl^−	1.36	2
Ru	RuO^− 4(aq) + 8 H^+ + 5 e^−	⇌	Ru^2+ (aq) + 4H2O	1.368	5
Ru	RuO 4 + 4 H^+ + 4 e^−	⇌	RuO 2 + 2H2O	1.387	4
Co	CoO 2(s) + 4 H^+ +  e^−	⇌	Co^3+ + 2H2O	1.42	1
N	2NH 3OH^+ +  H^+ + 2 e^−	⇌	N 2H^+ 5 + 2H2O	1.42	2
I	2HIO(aq) + 2 H^+ + 2 e^−	⇌	I 2(s) + 2H2O	1.44	2
Br	BrO^− 3 + 5 H^+ + 4 e^−	⇌	HBrO(aq) + 2H2O	1.447	4
Pb	β-PbO 2(s) + 4 H^+ + 2 e^−	⇌	Pb^2+ + 2H2O	1.46	2
Pb	α-PbO 2(s) + 4 H^+ + 2 e^−	⇌	Pb^2+ + 2H2O	1.468	2
Br	2BrO^− 3 + 12 H^+ + 10 e^−	⇌	Br 2(l) + 6H2O	1.48	10
At	HAtO3 + 4 H^+ + 4 e^−	⇌	HAtO + 2H2O	1.5	4
Mn	MnO^− 4 + 8 H^+ + 5 e^−	⇌	Mn^2+ + 4H2O	1.51	5
O	HO^• 2 +  H^+ +  e^−	⇌	H 2O 2(aq)	1.51	1
Au	Au^3+ + 3 e^−	⇌	Au(s)	1.52	3
Ru	RuO^2− 4(aq) + 8 H^+ + 4 e^−	⇌	Ru^2+ (aq) + 4H2O	1.563	4
N	2NO(g) + 2 H^+ + 2 e^−	⇌	N2O(g) + H2O(l)	1.59	2
Ni	NiO 2(s) + 2 H^+ + 2 e^−	⇌	Ni^2+ + 2 OH^−	1.59	2
Ce	Ce^4+ +  e^−	⇌	Ce^3+	1.61	1
Cl	2HClO(aq) + 2 H^+ + 2 e^−	⇌	Cl 2(g) + 2H2O	1.63	2
I	IO^− 4 + 2 H^+ + 2 e^−	⇌	IO^− 3 + H2O	1.64	2
Ag	Ag 2O 3(s) + 6 H^+ + 4 e^−	⇌	2Ag^+ + 3H2O	1.67	4
Cl	HClO 2(aq) + 2 H^+ + 2 e^−	⇌	HClO(aq) + H2O	1.67	2
Pb	Pb^4+ + 2 e^−	⇌	Pb^2+	1.69	2
Mn	MnO^− 4 + 4 H^+ + 3 e^−	⇌	MnO 2(s) + 2H2O	1.7	3
Br	BrO^− 4 + 2 H^+ + 2 e^−	⇌	BrO^− 3 + H2O	1.74	2
Ag	AgO(s) + 2 H^+ +  e^−	⇌	Ag^+ + H2O	1.77	1
N	N2O(g) + 2 H^+ + 2 e^−	⇌	N2(g) + H2O(l)	1.77	2	[6]: 789
O	H 2O 2(aq) + 2 H^+ + 2 e^−	⇌	2H2O	1.78	2
Au	Au^+ +  e^−	⇌	Au(s)	1.83	1
Co	Co^3+ +  e^−	⇌	Co^2+	1.92	1
Ag	Ag^2+ +  e^−	⇌	Ag^+	1.98	1
O	S 2O^2− 8 + 2 e^−	⇌	2SO^2− 4	2.01	2
O	O 3(g) + 2 H^+ + 2 e^−	⇌	O 2(g) + H2O	2.075	2
Mn	HMnO^− 4 + 3 H^+ + 2 e^−	⇌	MnO 2(s) + 2H2O	2.09	2
Xe	XeO 3(aq) + 6 H^+ + 6 e^−	⇌	Xe(g) + 3H2O	2.12	6
Xe	H 4XeO 6(aq) + 8 H^+ + 8 e^−	⇌	Xe(g) + 6H2O	2.18	8
Fe	FeO^2− 4 + 8 H^+ + 3 e^−	⇌	Fe^3+ + 4H2O	2.2	3
Xe	XeF 2(aq) + 2 H^+ + 2 e^−	⇌	Xe(g) + 2HF(aq)	2.32	2
O	HO• +  H^+ +  e^−	⇌	H2O(l)	2.38	1
Xe	H 4XeO 6(aq) + 2 H^+ + 2 e^−	⇌	XeO 3(aq) + 3H2O	2.42	2
F	F 2(g) + 2 e^−	⇌	2F^−	2.87	2
Cm	Cm^4+ + e^–	⇌	Cm^3+	3.0	1
F	F 2(g) + 2 H^+ + 2 e^−	⇌	2HF(aq)	3.077	2
Tb	Tb^4+ + e^–	⇌	Tb^3+	3.1	1
Pr	Pr^4+ + e^–	⇌	Pr^3+	3.2	1
Kr	KrF 2(aq) + 2 e^−	⇌	Kr(g) + 2F^− (aq)	3.27	2

See also

• Galvanic series lists electrode potentials in saltwater
• Standard apparent reduction potentials in biochemistry at pH 7
• Reactivity series#Comparison with standard electrode potentials

Notes

1. Not specified in the indicated reference, but assumed due to the difference between the value −0.454 and that computed by (2×(−0.499) + (−0.508))/3 = −0.502, exactly matching the difference between the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PH₃.

References

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External links

• Chemistry LibreTexts (2021-04-26). "P1: Standard Reduction Potentials by Element". Chemistry LibreTexts. Retrieved 2021-11-30.
• California State University, Northridge (CSUN). "Standard Reduction Potentials" (PDF). csun.edu. Archived (PDF) from the original on 2017-12-15. Retrieved 2021-11-30.
• Wardman, Peter (1989). "Reduction potentials of one-electron couples involving free radicals in aqueous solution" (PDF). srd.nist.gov. Archived (PDF) from the original on 2022-10-09. Retrieved 2021-11-30.
• http://www.jesuitnola.org/upload/clark/Refs/red_pot.htm Archived 2008-07-20 at the Wayback Machine
• https://web.archive.org/web/20150924015049/http://www.fptl.ru/biblioteka/spravo4niki/handbook-of-Chemistry-and-Physics.pdf
• http://hyperphysics.phy-astr.gsu.edu/Hbase/tables/electpot.html#c1